Asked by sarah
Given the reaction: H2SO4 = 2NaOH -> NaSO4 = 2H20.
Determine the # of moles of sulfuric acid id needed to completely react with 2.3 L of 0.5 M of NaOH. Then determine the concentration of the solution if 3.0 L of it are used instead.
Determine the # of moles of sulfuric acid id needed to completely react with 2.3 L of 0.5 M of NaOH. Then determine the concentration of the solution if 3.0 L of it are used instead.
Answers
Answered by
Steve
avoid typos in your formula:
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
2.3L of .5M NaOH contains 1.15 moles NaOH
Since 1 mole H2SO4 reacts with 2 moles NaOH, you will use only 0.575 moles of H2SO4.
The final solution will contain the leftover H2SO4 and a quite soluble Na2SO4. Not sure what the question is getting at.
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
2.3L of .5M NaOH contains 1.15 moles NaOH
Since 1 mole H2SO4 reacts with 2 moles NaOH, you will use only 0.575 moles of H2SO4.
The final solution will contain the leftover H2SO4 and a quite soluble Na2SO4. Not sure what the question is getting at.
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